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10 November, 17:27

How much 3.0M NaOH is needed to neutralize 30ml of 0.75M of H2SO4?

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Answers (1)
  1. 10 November, 21:04
    0
    15mL

    Explanation:

    Step 1:

    Data obtained from the question

    This includes the following:

    Molarity of the base (Mb) = 3M

    Volume of base (Vb) =.?

    Volume of acid (Va) = 30mL

    Molarity of the acid (Ma) = 0.75M

    Step 2:

    The balanced equation for the reaction.

    H2SO4 + 2NaOH - > Na2SO4 + 2H2O

    From the balanced equation above,

    The mole ratio of the acid (nA) = 1

    The mole ratio of the base (nB) = 2

    Step 3:

    Determination of the volume of the base.

    This can be achieved as follow:

    MaVa/MbVb = nA / nB

    0.75 x 30 / 3 x Vb = 1/2

    Cross multiply

    3 x Vb = 0.75 x 30 x 2

    Divide both side by 2

    Vb = (0.75 x 30 x 2) / 3

    Vb = 15mL

    Therefore, the volume of the base needed is 15mL.
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